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Ch. 1 - Matter I. States of Matter Kinetic Energy States of Matter A. Kinetic Energy Particles of matter are always in motion. The kinetic energy (speed) of these particles increases as temperature increases. B. Four States of Matter Solids very low KE - particles vibrate but can’t move around fixed shape fixed volume B. Four States of Matter Liquids low KE - particles can move around but are still close together Take the shape of the container fixed volume B. Four States of Matter Gases high KE - particles can separate and move throughout container variable shape variable volume B. Four States of Matter Plasma very high KE - particles collide with enough energy to break into charged particles (+/-) gas-like, variable shape & volume stars Another look at all the states of matter Ch. 1 - Matter II. Matter Flowchart Pure Substances Mixtures A. Matter Flowchart MATTER yes MIXTURE yes Is the composition uniform? Homogeneous Mixture (solution) PURE SUBSTANCE no Heterogeneous Mixture Colloids no Can it be physically separated? yes Can it be chemically decomposed? Compound Suspensions no Element A. Matter Flowchart Examples: graphite element pepper hetero. mixture sugar (sucrose) compound paint homo. mixture soda solution B. Pure Substances Element composed of identical atoms EX: copper wire, aluminum foil B. Pure Substances Compound composed of 2 or more elements in a fixed ratio properties differ from those of individual elements EX: table salt (NaCl) C. Mixtures Combination of 2 or more pure substances. Heterogeneous Homogeneous C. Mixtures Solution homogeneous very small particles particles don’t settle EX: rubbing alcohol C. Mixtures Colloid heterogeneous medium-sized particles particles don’t settle EX: milk C. Mixtures Suspension heterogeneous large particles particles settle EX: fresh-squeezed lemonade C. Mixtures Examples: mayonnaise colloid muddy water suspension fog colloid saltwater solution Italian salad dressing suspension Ch. 1 - Matter III. Properties & Changes in Matter Extensive vs. Intensive Physical vs. Chemical A. Extensive vs. Intensive Extensive Property depends on the amount of matter present Intensive Property depends on the identity of substance, not the amount A. Extensive vs. Intensive Examples: boiling point intensive volume extensive mass extensive density intensive conductivity intensive B. Physical vs. Chemical Physical Property can be observed without changing the identity of the substance Chemical Property describes the ability of a substance to undergo changes in identity B. Physical vs. Chemical Examples: melting point physical flammable chemical density physical magnetic physical tarnishes in air chemical B. Physical vs. Chemical Physical Change changes the form of a substance without changing its identity properties remain the same Chemical Change changes the identity of a substance products have different properties B. Physical vs. Chemical Signs of a Chemical Change change in color or odor formation of a gas formation of a precipitate (solid) change in light or heat B. Physical vs. Chemical Examples: rusting iron chemical dissolving in water physical burning a log chemical melting ice physical grinding spices physical How would you separate the following mixture? IRON FILINGS, SALT, CHALK POWDER AND WATER Dissolve as much of the mixture as possible Add water and stir Filter the mixture so that the soluble salt will be obtained in the filtrate and the insoluble chalk powder will be the residue on the filter paper Place the dry mixture into a beaker Dry out the filter paper to keep the dry chalk powder Use a magnet to attract and extract the iron filings from the dry mixture Pour the filtrate into an evaporating basin to evaporate the water and leave behind the salt